JC H1 A Level Chemistry Syllabus
Chemistry: Syllabus 8873. (First year of examination in 2026)
About the Syllabus: The enhanced syllabus for the A Levels aims to teach and impart 3 key qualities or “practices of science” to aspiring students. These include:
- Ways of Thinking and Doing in Science (WOTD) – Scientific inquiry involves investigating (posing questions, designing experiments, analyzing data), evaluating and reasoning (defending ideas with evidence, making informed decisions), and developing explanations (using models and constructing solutions).
- Nature of Scientific Knowledge (NOS) – Science builds evidence-based models to understand reality, assumes natural order, follows established procedures, and remains open to change with new evidence.
- Science-Technology-Society-Environment (STSE) – Science is interconnected with society, technology, and the environment, with applications having ethical, social, economic, and environmental impacts, often driving technological advancements.
H1 A Level Chemistry Syllabus Content
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• The nucleus of the atom: neutrons and protons, isotopes, proton and nucleon numbers • Electrons: electronic energy levels, ionisation energies, atomic orbitals, extranuclear structure
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• Ionic bonding, metallic bonding, covalent bonding and co-ordinate (dative covalent) bonding • Shapes of simple molecules and bond angles • Bond polarities and polarity of molecules • Intermolecular forces, including hydrogen bonding • Bond energies and bond lengths • Lattice structure of solids • Bonding and physical properties
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Theories of Acid and Bases |
• Arrhenius and Brønsted-Lowry theories of acids and bases • Acid dissociation constants, Ka • Base dissociation constants, Kb • The ionic product of water, Kw • pH: choice of indicators • Buffer solutions
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• Periodicity of atomic and physical properties of the elements: variation with proton number across the third period (sodium to chlorine) and down Group 17 of: (i) electronic configuration (ii) atomic radius and ionic radius (iii) ionisation energy (iv) electronegativity (v) melting point (vi) electrical conductivity • Periodicity of chemical properties of the elements in the third period: (i) variation in oxidation number and bonding of the oxides (sodium to sulfur only) and of the chlorides (sodium to phosphorus only) (ii) reactions of these oxides and chlorides with water (iii) acid/base behaviour of these oxides and the corresponding hydroxides • Periodicity of chemical properties of the elements down the group (Group 1 and Group 17): (i) as reducing agents (Group 1) and oxidising agents (Group 17) (ii) thermal stability of Group 17 hydrides
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The Mole Concept and Stoichiometry |
• Relative masses of atoms and molecules • The mole, the Avogadro constant • The calculation of empirical and molecular formulae • Reacting masses and volumes (of solutions and gases) • Redox processes: electron transfer and changes in oxidation number (oxidation state)
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Chemical Energetics: Thermochemistry |
• Enthalpy changes: ∆H, of formation; combustion; neutralisation; bond energy; lattice energy • Hess’ Law
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• Simple rate equations; orders of reaction; rate constants • Concept of activation energy • Effect of concentration, temperature, and catalysts on reaction rate • Heterogenous catalysts • Enzymes as biological catalysts
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• Chemical equilibria: reversible reactions; dynamic equilibrium (i) factors affecting chemical equilibria
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Polymers and Organic Chemistry
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• Empirical, molecular and structural formulae • Functional groups and the naming of organic compounds • Common terms for organic reactions • Isomerism: constitutional (structural); cis-trans • Shapes of organic molecules; σ and π bonds • Alkanes (as exemplified by ethane) (i) combustion and substitution reaction • Alkenes (as exemplified by ethene) (i) combustion and addition reactions • Halogenoalkanes (as exemplified by bromoethane) (i) substitution (ii) elimination • Alcohols (as exemplified by ethanol) (i) combustion (ii) oxidation to carboxylic acids (iii) elimination • Aldehydes (as exemplified by ethanal) (i) oxidation to carboxylic acid (ii) reduction • Ketones (as exemplified by propanone) (i) reduction • Carboxylic acids (as exemplified by ethanoic acid) (i) ester formation (ii) amide formation • Amino acids (as exemplified by aminoethanoic acid) • Structure and uses of polymers
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